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Related Concept Videos

Hydrogen Bonds00:26

Hydrogen Bonds

134.3K
Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....
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Hydrogen Bonds01:04

Hydrogen Bonds

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A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
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Intermolecular Forces03:13

Intermolecular Forces

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Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
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Intermolecular Forces in Solutions02:28

Intermolecular Forces in Solutions

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The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external source.
When the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change. Such a solution is called an ideal solution. A mixture of ideal gases (or gases such as helium and argon,...
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Intermolecular vs Intramolecular Forces03:00

Intermolecular vs Intramolecular Forces

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Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular force is influenced by the distance of separation between molecules. The forces significantly affect the interactions in solids and liquids, where the molecules are close together. In gases, IMFs become important only under high-pressure conditions (due to the proximity of gas molecules). Intermolecular forces dictate the physical properties of...
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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility02:34

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

51.7K
Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
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A Functionalized Heterocubane with Extensive Intermolecular Hydrogen Bonds.

Musa A Said1, Herbert W Roesky1, Carsten Rennekamp1

  • 1Institut für Anorganische Chemie der Universität, Tammannstrasse 4, D-37077 Göttingen (Germany), Fax: (+49) 551-393-337.

Angewandte Chemie (International Ed. in English)
|May 2, 2018
PubMed
Summary
This summary is machine-generated.

Cage compound 1 forms a unique 3D assembly via eight hydrogen bonds, creating molecular cavities. Compound 2, despite a similar structure, does not exhibit this crystal behavior.

Keywords:
Cage compoundsHydrogen bondsSilicon

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Area of Science:

  • Crystal engineering
  • Supramolecular chemistry
  • Materials science

Background:

  • Understanding the factors governing crystal packing and self-assembly is crucial for designing novel materials.
  • Hydrogen bonding interactions play a significant role in directing the formation of ordered structures in the solid state.

Purpose of the Study:

  • To investigate the crystal structure and self-assembly behavior of cage compound 1.
  • To compare the solid-state behavior of compound 1 with the structurally similar compound 2.

Main Methods:

  • Single-crystal X-ray diffraction analysis was employed to determine the three-dimensional structures of both compounds.
  • Analysis of intermolecular interactions, specifically hydrogen bonding, was performed.

Main Results:

  • Compound 1 exhibits a unique three-dimensional assembly in the crystal lattice.
  • Each molecule of compound 1 forms eight O-H⋅⋅⋅O hydrogen bonds with neighboring molecules.
  • These hydrogen bonds lead to the formation of cavities with approximate dimensions of 3×3×8 ų.
  • Compound 2, possessing the same framework structure, does not display similar hydrogen bonding or self-assembly behavior in the crystal.

Conclusions:

  • The specific arrangement of hydrogen bonds dictates the observed three-dimensional assembly in compound 1.
  • Subtle differences in molecular structure or environment can significantly alter self-assembly pathways, as seen by comparing compounds 1 and 2.